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Strong Acids and Bases

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Wize University Chemistry Textbook > Buffers and Titrations

Titration Problems

2 Activities

Wize University Chemistry Textbook > Acids and Bases

pH

4 Activities

Calculate the pH of a basic solution prepared by taking 10.00 mL of 0.700 M NaOH solution and diluting it to 100.00 mL with water.
More Titration Problems Questions:
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Acids and Bases: Titrations
25mL of a solution of 0.5mol/L KOH is required to neutralize 15mL of sulphuric acid. What is the concentration of the acid?
2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(ℓ)2KOH\left(aq\right)+H_2SO_4(aq)\to K_2SO_4(aq)+2H_2O(\ell)
Henderson Hasselbalch: Titrations and pH
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH (For ammonia Kb​=1.8×10−5)(For\ ammonia\ Kb​=1.8\times10^{-5})
Before the addition of any HCl
After 20.00 mL of the acid has been added
Redox
A 5.000 mL sample of a solution of hydrogen peroxide, H2O2, was analyzed by titration with potassium permanganate, KMnO4, according to the reaction shown below. The H2O2 sample required 42.8 mL of 0.0175 mol L−1 KMnO4 (aq) to reach the end point.
2 KMnO4 + 5 H2O2 + 6 H+ → 5 O2 + 2 Mn2+ + 2 K+ + 8 H2O
What was the concentration of the H2O2 solution? Choose the closest value.
To a 100 mL of 0.1M of CH3COOH\rm CH_3COOH (acetic acid) is added 25mL of 0.17M NaOH\rm NaOH. The Ka\rm K_a of acetic acid is 1.8×10−51.8 \times 10^{-5}. Calculate the pH\rm pH of the solution. Please report your answer to two decimal places.
25L of a solution of 0.5M KOH is required to neutralize 15L of sulphuric acid. What is the concentration of the acid? Balance the equation if it is unbalanced.
KOH + H2SO4 --> K2SO4 + 2H2O
What volume of hydrochloric acid of 0.1M is required to neutralize 500mL at 0.5M sodium hydroxide?
HCl + NaOH --> NaCl + H2O
Titration Problem
We titrated 40mL of 0.2M HBr with 0.4M NaOH...
The pH meter indicated that the initial pH was 2.9, pH at the half equivalence point was 3.5, equivalence pt was at pH 8.9.
a) What is Ka for HBr?
What volume of 3.16 M H3PO4 solution is necessary to react with 27 mL of 0.18 M Mg(OH)2?
Acid Base Calculation
An impure sample of solid Na2CO3 was reacted with 0.1755 M HCl. A 0.2337 g solid sample required 15.55 mL of HCl solution.
Practice: Long Titration Problem
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH
Before the addition of any HCl
After 20.00 mL of the acid has been added
Acids and Bases: Strong Acid Mixture
Practice Question: Strong Base Mixture
Calculate the pH and pOH of a solution containing a mixture of 75.00 mL of 0.100 M HI and 25.00 mL of 0.250 M HClO4.
Buffers: Titration of Sodium Citrate
A student dissolves a sodium citrate (Na3C6H5O7; MW = 258.069 g/mol) tablet in 350.00 mL of water. The student then pipetted 20.00 mL of the solution and performed a titration using a stock solution of HCl previously standardized to a concentration of 0.9899 M. The experiment required 33.55 mL of the HCl solution to reach the endpoint and fully neutralize the sodium citrate solution. Calculate the concentration of the sodium citrate solution.
Titrations
A student prepares a potassium hydrogen phosphate (K2HPO4, MW = 156.1739 g/mol) solution and pipettes 20.00 mL of this solution for a titration. In the titration, it required 23.43 mL of 0.100 M HCl to reach the endpoint. What is the concentration of the potassium hydrogen phosphate solution?
Titrations
A student prepares a potassium hydrogen phosphate (K2HPO4, MW = 156.1739 g/mol) solution and pipettes 20.00 mL of this solution for a titration. In the titration, it required 17.51 mL of 0.09977 M HCl to reach the endpoint. What is the concentration of the potassium hydrogen phosphate solution?
pH: Neutralization
A student adds 11.6 mL of a 3.7M KOH solution, to 29 mL of a 1.4 M HCl. What is the final pH after the addition?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Chemical Reactions: Limiting Reagent
15mL of a 1.2M solution of HCl reacts with 22mL of a 1.4M solution of NaOH. How many moles of NaOH are left after the reaction is complete?
HCl(aq)+NaOH(aq)→H2O(l)+NaCl(aq)HCl_{(aq)}+NaOH_{(aq)}\rightarrow H_2O_{(l)}+ NaCl_{(aq)}
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH. Enter 2 decimal places with all answers. Kb=1.8x10-5
Before the addition of any HCl
After 20.00 mL of the acid has been added
Acids and Bases: Titrations
25L of a solution of 0.5M KOH is required to neutralize 15L of sulphuric acid. What is the concentration of the acid? Balance the equation if it is unbalanced.
KOH + H2SO4 --> K2SO4 + 2H2O
Acids and Bases: Titrations
What volume of hydrochloric acid of 0.1M is required to neutralize 500mL at 0.5M sodium hydroxide?
HCl + NaOH --> NaCl + H2O
For which type of titration will the pH be basic at the equivalence point?
A student titrated 10.00 mL of 0.10 M sodium acetate (CH3COONa) with HCℓ and determined that 10.00 mL of HCℓ was needed to reach the equivalence point. At equivalence, what is the expected pH?
Ka of CH3COOH = 1.8×10-5
A student titrated 10.00 mL of 0.10 M sodium acetate (CH3COONa) with HCℓ and determined that 10.00 mL of HCℓ was needed to reach the equivalence point. At equivalence, what is/are the major species in solution (besides water and any pH-neutral ions)?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Henderson Hasselbalch: Titrations
Suppose you performed a potentiometric titration on the solutions in flasks A, B, and C by a gradual addition of HCℓ (aq) to each flask shown.
More pH Questions:
Weak Acids and Bases
Calculate the pH of the following solution.
A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Note: Acetic Acid Ka = 1.8 x 10-5
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a) A 6.30 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Methyl diethanolamine CH3N(C2H4OH)2 is a weak base which we will abbreviate as mdea. The conjugate acid, mdeaH+, has a pKa = 8.52.
Henderson Hasselbalch: Titrations and pH
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH (For ammonia Kb​=1.8×10−5)(For\ ammonia\ Kb​=1.8\times10^{-5})
Before the addition of any HCl
After 20.00 mL of the acid has been added
Molecular formula: Concentration
A solution of HBr has a pOH of 12.2, what is the [H+] concentration?
100 mL of a 0.5 M solution of nitric acid (HNO3\rm HNO_3) was added to 75 mL of a 0.37 M solution of sodium benzoate (C6H5COONa\rm C_6H_5COONa) the conjugate base of benzoic acid (C6H5COOHKa=6.6×10−5\rm C_6H_5COOH Ka = 6.6 \times 10^{-5}). Calculate the pH\rm pH of the resulting solution.
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution
Acids and Bases: pH of Alkaline Earth Metal Hydroxides
Calculate the pH of a 1.00 x 10-4 M Mg(OH)2 solution.
Acids and Bases: Strong Acid Mixture
Practice Question: Strong Base Mixture
Calculate the pH and pOH of a solution containing a mixture of 75.00 mL of 0.100 M HI and 25.00 mL of 0.250 M HClO4.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.500 g of sodium hydrogen phosphate (Na2HPO4, MW = 141.9579 g/mol) in 150.0 mL of water.
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a) A 6.30 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Strong Acids and Bases
Calculate the pH of a solution prepared by adding 100.0 mL of 3.00 x 10-2 M KOH with 50.0 mL of 2.50 x 10-2 M Be(OH)2.
Strong Acids and Bases
Calculate the pH and pOH of the following solutions.
a) 2.75 x 10-3 M aqueous HNO3 solution.
b) 1.50 x 10-2 g of CaO dissolved in 200.0 mL of water.
Weak Acids and Bases
Calculate the pH and pOH of the following solutions, knowing that Ka = 1.8x10^-5.
a) A 5.33 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 1.15 x 10-3 g of CH3COONa in 100.0 mL of water.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.150 g of sodium hydrogen phosphate (Na2HPO4, MW = 141.9579 g/mol) in 125.0 mL of water.
Ka (HPO42−) = 4.2 x 10−13;  Kb (HPO42−) = 1.6 x 10−7. K_a\ \left(HPO_4^{2-}\right)\ =\ 4.2\ x\ 10^{-13};\ \ K_b\ \left(HPO_4^{2-}\right)\ =\ 1.6\ x\ 10^{-7}.\
Strong Acids and Bases
Calculate the pH of a basic solution prepared by taking 20.00 mL of 0.500 M Be(OH)2 solution and diluting it to 100.00 mL with water.
Strong Acids and Bases
Calculate the pH of a solution prepared by adding 25.00 mL of 0.100 M HCl with 75.00 mL of 2.50 x 10-2 M HBr.
Strong Acids and Bases
Calculate the pH and pOH of the following solutions.
a) 3.00 x 10-4 M aqueous HClO4 solution.
b) 8.00 x 10-3 g of Na2O dissolved in 150.0 mL of water.
Consider the following reaction in water:
NaOH <----> Na+ + OH-
This reaction has a Kb of 1 x 10-10 and a pOH of 3. If there is 1 M of NaOH at equilibrium, what is the concentration of Na+ in solution?
Acids and Bases: pH based on % dissociation
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution
If an answer is an exponent such as 4.3x10-7, input the answer as: 4.3e-7
Which of the solutions below would have the HIGHEST pH value?
Acids and Bases: pH
What is the pH of a 0.10 M solution of NaF? (Ka for HF = 6.8×10-4)?
Methyl diethanolamine CH3N(C2H4OH)2 is a weak base which we will abbreviate as mdea. The conjugate acid, mdeaH+, has a pKa = 8.52.